Question 21 (4 points) What is the expression for the equilibrium constant for the following system?...
a. What is the equilibrium constant expression for the reaction: 3 Fe (s) + 4 H2O (g) + Fe3O4 (s) + 4 H2 (g) b. The equilibrium constant, Kc, for the reaction 2 NOCI (9) ++ 2 NO (g) + Cl2 (g) is 2.4 x 10-7. What is the Kc for the reaction: 1/3 Cl2 (g) + 2/3 NO (g) ++2/3 NOCI (g)
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
15. This question has multiple parts. Work all the parts to get the most points. At 35°C, K-1.1 x 10° for the reaction 2 NOCI(g) 근 2N0(g) + Cl2 (g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures a3.8 moles of pure NOCl in a 2.0-L flask [NOCI] = NO] [C12] = b1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask NOCI NO Numeric input field 3.8 mole of...
Write the expression for the equilibrium constant K, for the following reaction. (Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH)2 as (P NH3)2. If either the numerator or denominator is 1, please enter 1.) 2 NOCI() H 2NO(g) + Cl2(g) K = -
What is the equilibrium equation for the reaction? SIC14 (8) + 2 H2(g) Si (s) + 4 HCI (8) OK [Si]+[C] [SIC]2[H2] K [51][HC14 [SiC14][H2) Kc [HC14 [H2)” [Sicla] KC [S1C14][H.] [Si] [#C?*
For each of the following reactions choose the expression that represents Kc for the reaction: 1) TlCl3(s) TlCl(s) + Cl2(g) a) Kc = [TlCl3]/[TlCl][Cl2] b) Kc = [TlCl][Cl2]/[TlCl3] c) Kc = [Cl2] 2) CuCl42-(aq) Cu2+(aq) + 4Cl-(aq) a) Kc = [Cu2+][Cl-]4/[CuCl42-] b) Kc = [Cu2+][Cl-]/[CuCl42-] c) Kc = [CuCl42-]/[Cu2+][Cl-] 3) 3O2(g) 2O3(g) a) Kc = [O2]3/[O3]2 b) Kc = [O3]3/[O2]2 c) Kc = [O3]2/[O2]3 4) 4H3O+(aq) + 2Cl-(aq) + MnO2(s) Mn2+(aq) + 6H2O(ℓ) + Cl2(aq) a) Kc = [Mn2+][Cl2]/[H3O+]4[Cl-]2 b)...
1. Write the equilibrium-constant expression (Kc) for the following reactions (a) H2 (g) + 12(g) = 2H1 (9) (b) 2Cl2 (g) + 2H20 (9) + 4HCI (9)+ O2 (g) (c) H2(g) + Br2(1) HBr (g) (d) Ag(CN) 2 (aq) + Agl (s) + (aq) + 2AgCN (s)
Which of the following is the equilibrium constant expression for the reaction: 2NO(g) + O2(g) - 2NO2(8) [NO] A. Kod [NO] [02] [no] [NO] [02] [NO] [NOJ +[02] 2[NO] D. K. INO]+[02] E. None of the choices are correct. Option A Option B
Consider the equilibrium reaction and its equilibrium constant expression. *_ [ICI 12(g) + Cl () = 2ICI(g) [12] [CL] For the reaction 21C1(g) = 12(8) + C1,(8) select the equilibrium constant explossion. O x _ [L] [C12] [ICI) 2 [ICI] OK' =
The equilibrium constant, K, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g) + Cl2(8) = 2NOCI(g) is 6.5 x 104 at 35°C. In which direction will the reaction proceed to reach equilibrium if the starting concentrations of NO, Cl., and NOCI are 2.6 x 10-3 M, 7.4 x 10-M, and 5.8 M respectively? o o O shift right shift lent neither